A solution of 0.100 M HCl and a solution of 0.100 M NaOH are prepared. A 40.0 mL sample of one of the solutions is added to a beaker and then titrated with the other solution. A pH electrode is used to obtain the data that are plotted in the titration curve shown.Identify the solution that was initially added to the beaker and which solution was in the buret. Explain your reasoning. 2.At the equivalence point, how many moles of titrant have been added? 3.The same titration is to be performed again, this time using an indicator. Use the information in the table below to select the best indicator for the titration. Explain your choice. 1412-10-8.pH6.4-2.0-20.040.060.080.0Volume of Titrant Added (mL)pH Range ofColor ChangeIndicatorce.се.Methyl violet0- 1.6Methyl red4 -6Alizarin yellow10 – 12

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Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.21QAP

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A solution of 0.100 M HCl and a solution of 0.100 M NaOH are prepared. A 40.0 mL sample of one of the solutions is added to a beaker and then titrated with the other solution. A pH electrode is used to obtain the data that are plotted in the titration curve shown.

Identify the solution that was initially added to the beaker and which solution was in the buret. Explain your reasoning.
2.At the equivalence point, how many moles of titrant have been added?

3.The same titration is to be performed again, this time using an indicator. Use the information in the table below to select the best indicator for the titration. Explain your choice.

14
12-
10-
8.
pH
6.
4-
2.
0-
20.0
40.0
60.0
80.0
Volume of Titrant Added (mL)
pH Range of
Color Change
Indicator
ce.
се.
Methyl violet
0- 1.6
Methyl red
4 -6
Alizarin yellow
10 – 12

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